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now in graphite each carbon atom us attached to 3 other carbon atoms because of which 1 electron of each atom is free ec of carbon is 2,4 these free electrons [in different layers] have very weak columns of forces between them [with one directy below it] of lenght about 335pm[pico metre]. 2 understand better check out the structure of graphite.
AA
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What type of covalent bonds does graphite have?
Graphite has covalent bonds known as sigma bonds between each carbon atom within a single layer, as well as delocalized pi bonds that extend across multiple layers. These pi bonds allow for the unique properties of graphite, including its lubricating and electrical conductivity properties.
What makes diamonds so strong and graphite so brittle and breakable?
The difference in strength between diamonds and graphite is due to their different atomic structures. Diamonds have a three-dimensional network of strong covalent bonds between carbon atoms, making them very hard. In contrast, graphite has layers of carbon atoms held together by weak van der Waals forces, allowing the layers to slide over each other easily, making graphite soft and brittle.
What type of bond is in graphite?
Graphite is made of covalent bonds, where carbon atoms share electrons to form strong bonds. This allows graphite to have a layered structure, with each layer held together by weak van der Waals forces.
Why does diamond have a greater density than graphite?
Diamond has a greater density than graphite because it has a crystal structure where each carbon atom is bonded to four other carbon atoms in a tetrahedral arrangement, making it tightly packed and more dense. In contrast, graphite has a layered structure with weak forces between the layers, resulting in a lower density.
Is KC8 the molecular formula of graphite?
No- KC8 (also known as "cake") is potassium-intercalated graphite. It is often used as a very powerful reducing agent in organometallic reactions. It is synthesized by melting potassium metal over graphite powder in an inert atmosphere and is highly pyrophoric.
What type of covalent bonds does graphite have?
Graphite has covalent bonds known as sigma bonds between each carbon atom within a single layer, as well as delocalized pi bonds that extend across multiple layers. These pi bonds allow for the unique properties of graphite, including its lubricating and electrical conductivity properties.
Why graphite is conductor as it is the form of carbon?
Unlike the other allotropes of carbon (such as diamond), in graphite, each carbon atom forms 3 strong bonds (rather than 4) with its neighbours. These form in layers of hexagons. Between each layer of hexagons, there are delocalised electrons, that form a weak bond with the next layer. This weakness is responsible for the use of graphite as a lubricant or in pencils (where one layer of graphite can easily slide over another). The delocalised electrons are also able to carry an electrical charge, because they can move freely.
Why graphite conduct electricity as other non metals do not?
Graphite has delocalised electrons. It has layer structure (each layer is called graphene). The bonding of the carbons in the layer can be described as sp2 as the bond angles are 120 0. Each C atom has a p orbital perpendicular to the layer that contains a single electron. These p orbitals form pi bonds which spread across the layer.
Number of adjacent carbon atom in graphite?
In graphite, each carbon atom is bonded to three other carbon atoms in a hexagonal lattice structure. This creates a 2D network of interconnected carbon atoms that form layers. Each carbon atom in graphite is adjacent to three other carbon atoms within the same layer.
What is the structural difference between a diamond and graphite?
The structural difference between diamond and graphite is in their arrangement of carbon atoms. Diamond has a three-dimensional network structure where each carbon atom is bonded to four other carbon atoms in a tetrahedral arrangement. In contrast, graphite consists of layers of carbon atoms arranged in hexagonal rings with each carbon atom bonded to three others in the same plane, allowing for easy slippage between the layers.
How do you Propose an explanation for the difference in propertise between diamond and graphite?
The difference in properties between diamond and graphite is primarily due to their distinct atomic structures. In diamond, each carbon atom is tetrahedrally bonded to four other carbon atoms, creating a strong three-dimensional network that results in high hardness and a brilliant luster. In contrast, graphite has a planar structure where each carbon atom is bonded to three others in flat sheets, with weaker van der Waals forces between the layers, allowing them to slide over each other. This structural variation accounts for diamond’s rigidity and brilliance compared to graphite’s softness and conductivity.
Why is graphite a good lubricant and diamond is an excellent abrasive?
Because graphite forms layers and each layer, each carbon molecule is bonded to three other carbon molecules. The fourth electron to each atom is weakly bonded to the layer next to it. The structure allows the layers to slide past each other, making this element an excellent lubricant.
What is the molecular structure of a pencil?
A pencil is primarily made of graphite, a crystalline form of carbon. The molecular structure of graphite is made up of layers of carbon atoms arranged in a hexagonal lattice structure, with each carbon atom bonded to three others in the same layer. These layers are held together by weak van der Waals forces, allowing the layers to slide past each other easily, giving graphite its lubricating properties.
What is lead in pencil?
Graphite is present in pencil leads. it is composed of carbon atoms covalently bonded with each other, and 1 free valence electron in each atom (which explains why graphite/pencil-lead conducts electricity)
How are carbon atoms bonded together in the graphite layer?
They are bonded by nonpolar covalent bonds. Each of the atoms is sp2 hybridized. It is sometimes depicted as having alternating single and double bonds, but this is not quite accurate. The bonds are subject to what is called resonance so that the bonds are neither single nor double but sort of in between.
How many atoms thick is graphene?
Graphene is a single layer of carbon atoms arranged in a two-dimensional honeycomb lattice, making it just one atom thick. This unique structure gives graphene its remarkable electrical, thermal, and mechanical properties. When multiple layers of graphene are stacked together, they form graphite, but each individual layer remains only one atom thick.
Is graphite is a good conductor of electricity?
Yes it is.
